A. Stoichiometry I
1. Balance the following equation and perform the following operations.
_____ NH3(g) + _____ NO (g) → _____ N2(g) + _____ H2O (l)
2. Using the balanced equation from above, perform the following stoichiometric
conversions.
a How many mol of NH3 are needed to completely react with 3.8 mol of NO?
● 3.8 mol NO → mol NH3
b. How many mol of NH3 are necessary for the production of 126 g of water?
● 126 g H2O → mol NH3
c. What mass of NO is consumed by the reaction of 71.0 g of NH3?
● 71.0 g NH3 → g NO
d. How many L of N2 are produced from the formation of 98.0 g of H2O?
● 98.0 g H2O → L N2
e. If 17 mol of NO are used, how many water molecules will be produced?
● 17 mol NO → atoms H2O

3. Essential ?’s
a. How can a balanced equation be used to determine relationships between
moles of reactants and moles of products? Explain.
b. Using the balanced chemical equation from V-A1 above, construct
(at least) 2 mol ratios and explain (briefly) the relationships (i.e. what are
you converting to and from).